acids and bases

Question 1

Arrhenius

Answer 1

Acid: increases [H3O+] hydronium
Base: increases [OH-] hydroxide

Question 2

Bronsted Lowry

Answer 2

Acid: donates proton
Base: accepts proton

Question 3

Lewis

Answer 3

in the formation of covalent bonds

Acid: accept electron pairs
Base: donates electron pairs

Question 4

conjugate acids and bases

Answer 4

base: mawawalan ng isang h mag -1 charge

acid: madadagdagan h +1 charge

Question 5

strong acid and weak acid value of Ka

Answer 5

strong: large Ka&raquo_space; 1
weak: small Ka &laquo_space;1

Question 6

Water dissociates very slightly into ions in an equilibrium

Answer 6

autoionization or self-ionization

Question 7

Water ionizes to produce both H3O+ and OH-, thus it
has

Answer 7

both acid and base properties.

Question 8

Kw is called water
ionization constant.

Answer 8

1.0 x 10-14 at 25oC

Question 9

present in all aqueous systems

Answer 9

hydronium and hydroxide

Question 10

We can define the terms “acidic” and “basic” in terms of
the relative concentrations of H3O+ and OH– ions

Answer 10

In an acidic solution,
[H3O+] >[OH–]

In a neutral solution,
[H3O+] =[OH–]

In a basic solution,
[H3O+] < [OH–]

Question 11

The pH of a solution indicates its relative acidity

Answer 11

In an acidic solution,
pH <7.00

In a neutral solution,
pH =7.00

In a basic solution,
pH > 7.00

Question 12

formula for pH

Answer 12

pH = -log[H3O+]

Question 13

If [H3O+] increases,

Answer 13

[OH–] decreases

Question 14

pKw =

Answer 14

pH + pOH at any temp

= 14.00 at 25°C

Question 15

the number of decimal places in
the pH equals

Answer 15

the number of significant
figures in the hydrogen-ion concentration.

Question 16

acidic, basic, neutral based on M

Answer 16

Acidic solutions:
[H3O+] > 1.0 x 10-7 M;

Basic solutions:
[OH-] > 1.0 x 10-7 M

Neutral solutions:
[H3O+] = [OH-] = 1.0 x 10-7 M

Question 17

percent ionization formula

Answer 17

M ionized / M initial x 100